What Is an Oxidizing Agent?
The property of the oxidant to obtain electrons is called oxidizing property, and the determinant factor of the oxidizing property is the electron-producing tendency of the high-valent element in the substance. In solution, according to the theory of electric double layer, the size of oxidizing power is reflected by the standard hydrogen electrode potential of oxidizing agent: the higher the potential, the stronger the oxidizing power; the lower the potential, the weaker the oxidizing power, correspondingly, its reduced state The stronger the reducibility. Strong oxidants are oxidizing substances with high potential.
Strong oxidants
English name: strong oxidant
Has a strong
Weak oxidant | With Fe3 + ions as the limit, the standard electrode potential value is less than 0.77 (E <0.77V) | Hydrogen ion H + (0); sulfur S (0.142); normal tetravalent tin ion Sn4 + (0.151); positive trivalent antimony ion Sb3 + (0.152); dilute sulfuric acid H2SO4 (0.17); positive divalent copper ion Cu2 + (0.341); positive tetravalent sulfur Ions S4 + (0.45); positive monovalent copper ion (copper ion) Cu1 + (0.52); iodine I2 (0.536) |
Strong oxidant | Electrode potential from Fe3 + ions to O2 oxygen (+ 0.77V <E <+ 1.23V) | Positive trivalent iron ion Fe3 + (0.77); positive monovalent mercury ion (mercury ion) Hg + (0.79); positive monovalent silver ion Ag + (0.8); positive divalent mercury ion Hg2 + (0.85); cold concentrated sulfuric acid H2SO4 (0.9) Dilute nitric acid HNO3 (0.96); nitrous acid HNO2 (0.983); telluric acid H6TeO6 (1.02); tetravalent nitrogen ion N4 + (1.035); bromine Br2 (1.087); hot concentrated sulfuric acid H2SO4 (1.1); concentrated nitric acid HNO3 (1.1 ); Selenic acid H2SeO4 (1.15); carbon tetrachloride CCl4 (1.18); iodic acid HIO3 (1.195); tetravalent manganese ion Mn4 + (1.22) |
Very strong oxidant | From oxygen to Co3 + ions (+ 1.23V <E <+ 1.83V) | Oxygen O2 (1.23); trivalent tritium ions Tl3 + (1.25); dichromic acid H2Cr2O7 (1.33), chlorine gas Cl2 (1.358); perchloric acid (perchloric acid) HClO4 (1.39); hypoiodic acid HIO (1.44); Chloric acid HClO3 (1.47), bromic acid HBrO3 (1.482); n-trivalent gold ion Au3 + (1.5); hypobromous acid HBrO (1.57); periodate (metaperiodate) H5IO6 (1.60); hypochlorite HClO (1.61); Chlorous acid HClO2 (1.645); Orthotetravalent nickel ion Ni4 + (1.678); Permanganic acid (permanganic acid) HMnO4 (1.679); Orthotetravalent lead ion Pb4 + (1.691); Positive monovalent gold ion (Asian Gold ion) Au + (1.692); Perbromic acid (perbromic acid) HBrO4 (1.763); Positive monovalent nitrogen ion N + (1.766); Hydrogen peroxide H2O2 (1.776, actual oxidation capacity is weaker than chlorine Cl2) |
Extremely strong oxidant | Oxidation is greater than Co3 + ion (E> + 1.83V) | Positive trivalent cobalt ion Co3 + (1.83); Positive divalent silver ion Ag2 + (1.98); Peroxodisulfate H2S2O8 (requires silver ion Ag + catalysis) (2.01); Ozone O3 (2.076); Xenonate H2XeO4 (2.11); Ferrate H2FeO4 ( 2.2); oxygen fluoride OF2 (2.244); xenon difluoride XeF2 (2.365); bromine pentafluoride BrF5 (2.408); oxygen atom O (2.694); chlorine trifluoride (2.796); ); Fluorine gas F2 (2.866); rhodium hexafluoride RhF6 (2.908); platinum hexafluoride PtF6 (2.924); iridium hexafluoride IrF6 (2.941); perfluorenic acid H4XeO6 (explosive decomposition when the concentration is> 8mol / L) (3.0); Dioxydifluoride (very unstable) (3.0194); Trioxydifluoride O3F2 (oxygen element is +2/3 valence) (3.0202); Hexaoxydifluoride O6F2 (very unstable) 3.0272); europium difluoride KrF2 (3.0273); fluorine atom F (3.055) |
1.
Common reducing agents are substances that are susceptible to oxidization of electrons in chemical reactions.
(1) Typical metal simple materials such as: K, Ca, Na, Mg, etc. (its reducing strength is basically consistent with metal activity)
(2) Certain non-metallic elements and their compounds such as: H2, C, CO.
(3) The lowest valence compounds with variable elements such as: H2S, HI, HBr, HCl
(4) Non-metallic anions such as: S2-, I-, Br-, Cl-
Lively metal elements such as Na, Al, Zn, Fe, etc. Some non-metallic elements, such as H2, C, Si, etc. Oxides when elements (such as C, S, etc.) are at low valence, such as CO, SO2, etc. Acids when elements (such as Cl, S, etc.) are at low valence, such as HCl, H2S, etc. Salts when elements (such as Fe, S, etc.) are at low valence, such as Na2SO3, FeSO4, etc.
Common reducing agents are: hydrogen (H2), carbon monoxide (CO), iron filings (Fe), zinc powder (Zn), and the like.
